Solubility and Stability of Carotenoids in Ammonium- and Phosphonium-Based Ionic Liquids: Effect of Solvent Nature, Temperature and Water

Ionic liquids (ILs) have arisen as alternatives to organic solvents and been used in natural pigment extraction in recent decades. However, the solubility and stability of carotenoids in phosphonium- and ammonium-based ILs are insufficiently explored. In this work, the physicochemical properties of the ILs, and the dissolution behavior and storage stability of three carotenoids (astaxanthin, β-carotene, and lutein) in the IL aqueous solution were investigated. The results showed that the solubility of the carotenoids in the acidic IL solution is higher than that in the alkaline IL solution, and the optimal pH is about 6. The solubility of astaxanthin (40 mg/100 g), β-carotene (105 mg/100 g), and lutein (5250 mg/100 g) was the highest in tributyloctylphosphonium chloride ([P4448]Cl) due to the van der Waals forces with [P4448]+ and hydrogen bonding with Cl−. A high temperature was beneficial to improve the solubility, but it can reduce the storage stability. Water has no significant effect on the carotenoid stability, but a high water content decreases the carotenoid solubility. A IL water content of 10–20%, an extraction temperature of 338.15 K, and a storage temperature of less than 298.15 K are beneficial for reducing the IL viscosity, improving carotenoid solubility, and maintaining good stability. Moreover, a linear correlation was found between the color parameters and carotenoid contents. This study provides some guidance for screening suitable solvents for carotenoid extraction and storage.


Introduction
Carotenoids are liposoluble compounds containing 40 carbon atoms with conjugated double bonds [1]. Carotenoids are divided into two main groups: carotenes and xanthophylls. Carotenes consist of hydrocarbon chains (e.g., α-carotene, β-carotene, and lycopene), and xanthophylls consist of oxygen as a functional group (e.g., astaxanthin, zeaxanthin, and lutein) [2,3]. Carotenoids have been widely used as colorants, antioxidants, and antiinflammatory agents in different areas, such as the pharmaceutical [4,5], cosmeceutical [6], food [7,8], and feed [9,10] industries. The antioxidant capacity of astaxanthin is the highest [11], and lutein minimizes macular degeneration [12,13]. Recently, increasing attention has been paid to the extraction of natural carotenoids from plant resources. Astaxanthin of 19.8% was extracted from Haematococcus pluvialis by using hydrochloric acid pretreatment followed by acetone extraction [14]. Carotenoids were effectively extracted by anhydrous acetone from persimmon peel and pulp at 40 • C, and the yields of β-cryptoxanthin and β-carotene reached 16,709.90 mg/100 g and 4479.07 mg/100 g, respectively [15]. However, organic solvent extraction methods have huge disadvantages, such as their volatility and unknown biological toxicity. Therefore, the creation of new extraction solvents for carotenoids remains an important challenge, despite considerable progress.
A promising alternative is the use of ionic liquids (ILs). ILs are molten salts formed by organic cations and organic or inorganic anions and have been widely used as solvents

Phase Behavior of IL-Water Systems
Compared with imidazolium-based ILs, ammonium-and phosphate-based ILs with higher shielded charges are presented in the literature as hydrophobic ILs, with some of them having a relatively high solubility in water. Herein, the phase behavior of the IL-water systems was measured at 298.15 K, and the apparent phase state for the ILwater systems is noted in Table 1 3 COO were insoluble when the water content exceeded 20%. In solid-liquid extraction, the solvent should maintain its stability at different temperatures. Therefore, the homogeneous phase of the IL-water mixtures was selected as the preliminary solvent system. " " indicates a miscible homogeneous phase, "×" indicates stratification without miscibility.

Physicochemical Properties of IL Aqueous Solutions
The data of the physicochemical properties (density, pH, viscosity, and conductivity) of the IL aqueous solutions at temperature from 298.15 K to 338.15 K in the presence of 10% to 50% water are summarized in Tables S1 and S2 and presented in Figure 1.

Density
The density difference of the IL/water mixture is of great significance to the operation of separation equipment in industry. The density of ILs is mainly dependent on the void size and molar volume [27]. The extraction efficiency of ILs is highly dependent on their immiscibility with water based on the density difference. As shown in Table S1, the density of all the studied ILs lied in the range of 0.9113 to 1.0483 g·cm −1 , which is a typical density range for ILs. It is worth noticing that the larger the cation radius of the IL, the lower its densities. For example, the densities of phosphonium-based ILs were smaller than ammonium-based ILs, and the density decreases with the increase in alkyl chain length. The densities of the ILs with different cations followed the trend [N 4444 ] + > [P 4444 ] + > [P 4448 ] + , and the ILs containing different anions followed the trend Br − > CF 3 COO − > Cl − . Even though CF 3 COO − has a higher molecular weight than Br − , the C=O bond in CF3COO − combines with water to form strong hydrogen bonds, resulting in a decrease in density [28].
The molar volume and isotropic coefficient of expansion of the ILs increased with rising temperature (Table S1), because the kinetic energy of molecules increased at higher temperatures [29]. The densities of the IL/water mixture (w water = 20%) decreases linearly with the increase in temperature. Similarly, the density values of the 1-butyl-3-methylimidazolium tetrafluoroborate ([C 4 mim][BF 4 ])/water mixture (w water = 0.0207, 0.0403, 0.0611 mol/kg) decreased with the rise in temperature from 293.15 K to 318.15 K [30]. Adding water resulted in a decrease in hydrogen bonds between molecules, which may be due to the reduced interaction as well as cation mobility.

Density
The density difference of the IL/water mixture is of great significance to the operation of separation equipment in industry. The density of ILs is mainly dependent on the void size and molar volume [27]. The extraction efficiency of ILs is highly dependent on their immiscibility with water based on the density difference. As shown in Table S1, the density of all the studied ILs lied in the range of 0.9113 to 1.0483 g·cm −1 , which is a typica density range for ILs. It is worth noticing that the larger the cation radius of the IL, the lower its densities. For example, the densities of phosphonium-based ILs were smaller than ammonium-based ILs, and the density decreases with the increase in alkyl chain length. The densities of the ILs with different cations followed the trend [N4444] + > [P4444] + > [P4448] + , and the ILs containing different anions followed the trend Br − > CF3COO − > Cl − Even though CF3COO − has a higher molecular weight than Br − , the C=O bond in CF3COO

Density
The density difference of the IL/water mixture is of great significance to the operation of separation equipment in industry. The density of ILs is mainly dependent on the void size and molar volume [27]. The extraction efficiency of ILs is highly dependent on their immiscibility with water based on the density difference. As shown in Table S1, the density of all the studied ILs lied in the range of 0.9113 to 1.0483 g·cm −1 , which is a typical density range for ILs. It is worth noticing that the larger the cation radius of the IL, the lower its densities. For example, the densities of phosphonium-based ILs were smaller than ammonium-based ILs, and the density decreases with the increase in alkyl chain length.

Density
The density difference of the IL/water mixture is of great significance to the operation of separation equipment in industry. The density of ILs is mainly dependent on the void size and molar volume [27]. The extraction efficiency of ILs is highly dependent on their immiscibility with water based on the density difference. As shown in Table S1, the density of all the studied ILs lied in the range of 0.9113 to 1.0483 g·cm −1 , which is a typical density range for ILs. It is worth noticing that the larger the cation radius of the IL, the lower its densities. For example, the densities of phosphonium-based ILs were smaller than ammonium-based ILs, and the density decreases with the increase in alkyl chain length. The densities of the ILs with different cations followed the trend [N4444] + > [P4444] + > [P4448] + , and the ILs containing different anions followed the trend Br − > CF3COO − > Cl − .

Density
The density difference of the IL/water mixture is of great significance to the operation of separation equipment in industry. The density of ILs is mainly dependent on the void size and molar volume [27]. The extraction efficiency of ILs is highly dependent on their immiscibility with water based on the density difference. As shown in Table S1, the density of all the studied ILs lied in the range of 0.9113 to 1.0483 g·cm −1 , which is a typical density range for ILs. It is worth noticing that the larger the cation radius of the IL, the lower its densities. For example, the densities of phosphonium-based ILs were smaller than ammonium-based ILs, and the density decreases with the increase in alkyl chain length. The densities of the ILs with different cations followed the trend [N4444] + > [P4444] + > [P4448] + , and the ILs containing different anions followed the trend Br − > CF3COO − > Cl − .

Density
The density difference of the IL/water mixture is of great significance to the operation of separation equipment in industry. The density of ILs is mainly dependent on the void size and molar volume [27]. The extraction efficiency of ILs is highly dependent on their immiscibility with water based on the density difference. As shown in Table S1, the density of all the studied ILs lied in the range of 0.9113 to 1.0483 g·cm −1 , which is a typical density range for ILs. It is worth noticing that the larger the cation radius of the IL, the lower its densities. For example, the densities of phosphonium-based ILs were smaller than ammonium-based ILs, and the density decreases with the increase in alkyl chain length.

Density
The density difference of the IL/water mixture is of great significance to the operation of separation equipment in industry. The density of ILs is mainly dependent on the void size and molar volume [27]. The extraction efficiency of ILs is highly dependent on their immiscibility with water based on the density difference. As shown in Table S1, the density of all the studied ILs lied in the range of 0.9113 to 1.0483 g·cm −1 , which is a typical density range for ILs. It is worth noticing that the larger the cation radius of the IL, the lower its densities. For example, the densities of phosphonium-based ILs were smaller than ammonium-based ILs, and the density decreases with the increase in alkyl chain length. The densities of the ILs with different cations followed the trend [N4444] + > [P4444] + > [P4448] + , and the ILs containing different anions followed the trend

Density
The density difference of the IL/water mixture is of great significance to the operation of separation equipment in industry. The density of ILs is mainly dependent on the void size and molar volume [27]. The extraction efficiency of ILs is highly dependent on their immiscibility with water based on the density difference. As shown in Table S1, the density of all the studied ILs lied in the range of 0.9113 to 1.0483 g·cm −1 , which is a typical density range for ILs. It is worth noticing that the larger the cation radius of the IL, the lower its densities. For example, the densities of phosphonium-based ILs were smaller than ammonium-based ILs, and the density decreases with the increase in alkyl chain length. The densities of the ILs with different cations followed the trend [N4444] + > [P4444] + > [P4448] + , and the ILs containing different anions followed the trend Br − > CF3COO − > Cl − .

Density
The density difference of the of separation equipment in indus size and molar volume [27]. The e immiscibility with water based on sity of all the studied ILs lied in density range for ILs. It is worth lower its densities. For example, than ammonium-based ILs, and length.  Figure 1).

pH
The acidity and alkalinity of the extraction system is are important factors for selecting extraction equipment. In general, the studied IL aqueous solution presented a wide range of pH values [31], approximately ranging from 1 to 11. The ILs with [P 4444 ] + or [P 4448 ] + cations were acidic, while the ILs with [N 4444 ] + cations were neutral or basic. It is noteworthy that the properties of ILs may depend on the strength of the interaction between the anion and water [32]. CF3COO − could form a relatively stable weak acid with H − from H 2 O, and promoted the ionization of H 2 O. Therefore, the highest pH value of 11.13 was for the mixture of [N 4444 ]CF 3 COO/water (w water = 20%, T = 338.15 K), and the lowest pH was 0.62 for the mixture of [P 4448 ]Cl/water (w water = 10%, T = 298.15 K).

Viscosity
In green extraction technology, solvents with a low viscosity have a stronger advantage. Dannie et al. [33] suggested a viscosity of 100 mPa·s −1 as the maximum viscosity value in process engineering research. In recent years, imidazolium-based ILs have become widely used extraction solvents [18]. However, due to their high viscosity, cosolvents such as water or organic solvents were often added to enhance the mass transfer [34]. Królikowska et al. [35] reported that the viscosity of ethylsulfate-based ILs decreased with an increasing amount of water in binary mixtures.
In this study, all viscosity values of ammonium-and phosphonium-based ILs (w water = 20%) were lower than 100 mPa·s −1 in the temperature range of 298. 15 4444 ]CF 3 COO. When the temperature was increased to 328.15 K or the water content was more than 30%, the viscosity values of the ILs were very close to each other. The van der Waals forces and hydrogen bonding between the anions and cations of the ILs were weakened when increasing the temperature and adding water [36,37]. Therefore, the viscosity of all the ILs decreased significantly with the increase in water content from 10% to 30%, and the lower viscosity of approximately 15 mPa·s −1 could be obtained with a water content of 30% at 338.15 K.

Conductivity
Conductivity, mainly related to the mobility of ions, is an essential parameter in evaluating aggregation behavior and the structure of solvents [38,39]. ILs with a higher viscosity exhibit a low conductivity. On the other hand, ILs with long alkyl chains have a lower conductivity than ILs with short alkyl chains, because the van der Waals force increases with the growth of the carbon chain [40]. Therefore, the conductivity of [P 4448 ]Br (w water = 10%) was the lowest of 2 mS·cm −1 at 298.15 K. A higher temperature and water content resulted in a reduction in the intermolecular force between the anions and cations of the ILs, which enhanced the ionization and ion mobility. As shown in Figure 1, the conductivity of all IL aqueous solutions significantly increased with the increase in temperature and water content. The conductivity of [P 4448 ]Br (w water = 10%) increased to 11.8 mS·cm −1 when the water content was 50%.

Solubility
Solubility behavior is the most challenging aspect for carotenoid extraction. The solvation properties of phosphonium-and ammonium-based ILs strongly depend on their structure and miscibility with water and can be tailored by changing the temperature. Therefore, the solubilities of carotenoids in [N 4444 15 K and water contents from 10% to 50%. The graphical results of solubility of astaxanthin, β-carotene, and lutein in IL aqueous solutions as a function of temperature (wwater = 20%) and water content (T = 298.15 K) are presented in Figure 2.  Generally, the solubility of the carotenoids in all studied ILs increased with the increase in temperature. The main reason may be that the viscosity of all ILs decreased significantly with the increase in temperature, as shown in Figure 1. On the other hand, the higher the water content in the ILs, the lower the viscosity. However, the solubility of the carotenoids decreased with the increase in water content. One potential explanation for the tendency might be that the anions and cations of the ILs were extremely solvated in excess water [41]. Similarly, the solubility of lamotrigine in aqueous mixtures of 1-octyl-3methylimidazolium bromide IL decreased with the increasing concentration of water [42]. However, it should be stressed that pure ILs showed a very high viscosity, which is not conducive to extraction applications. For example, the viscosity of [P 4448 ]Cl free of water at 298.15 K was 1260.0 mPa·s −1 , which was 18.5 times the viscosity in the presence of 10% water (68.0 mPa·s −1 ). Therefore, increasing the temperature to 328.15 K and adding water up to 20% are very necessary and beneficial to obtain a higher solubility of carotenoids in phosphonium-and ammonium-based ILs.
Moreover, the phosphonium-based ILs presented a stronger ability than ammoniumbased ILs to dissolve carotenoids. In particular, the ILs with Cl-showed a stronger solubility than the ILs with CF 3 COO − , and the ILs with longer alkyl chains facilitated the solubilization of carotenoids. Longer cationic alkyl side chains of the ILs resulted in stronger molecular vibrations, while a smaller ionic radius of anions resulted in more ions being transported and weaker van der Waals forces. Therefore, it could be observed that [P 4448 ]Cl showed the highest solubility for carotenoids, while [N 4444 ]CF 3 COO showed the lowest solubility. The solubilities of astaxanthin, β-carotene, and lutein in [P 4448 ]Cl at 338.15 K and 20% water content were approximately 40 mg/100 g, 105 mg/100 g, and 5250 mg/100 g, respectively, which was 10 times that in [N 4444 ]CF 3 COO. In addition, the solubility of different carotenoids in the ILs followed the trend lutein >> β-carotene-> astaxanthin. Lutein was highly polarized, and the solubility was hundreds of times higher than that reported in [43].
Methanol, ethanol, and acetone were the common organic solvents for natural dissolution and extraction [44]. The dissolution capacity of the methanol, ethanol, acetone were 0.02 mg/mL, 0.02 mg/mL, and 0.35 mg/mL at 35 • C, respectively [45]. Microemulsions had a large solubilization capacity for both hydrophilic and lipophilic compounds [46]. The solubilities of astaxanthin and lutein were 0.27 mg/mL and 12.50 mg/mL, respectively, in microemulsions composed of deep eutectic solvents (DL-menthol:acetic acid = 1:2), tween 80, and water [45]. In our study, the solubilities of astaxanthin and lutein in [P 4448 ]Cl at 35 • C and 20% water content were 0.07 mg/mL and 15.07 mg/mL, respectively. These results indicate that [P 4448 ]Cl aqueous solutions are good substitutes for organic solvents to improve the dissolution of carotenoids.

Interaction Force of Carotenoids with ILs
DFT studies allow us to interpret the mechanism of ILs with carotenoids, bonding types, and the strength of the bonding in the considered IL-carotenoid systems. Figure  S1 shows the optimized scatter diagrams of [P 4448 ] + -carotenoid, Cl − -carotenoid, and [P 4448 ]Cl − -carotenoid structures. To explore the interaction forces, the interactions between ions and carotenoids were investigated using the reduced density gradient (RDG) and independent gradient model (IGM). The RDG analysis can distinguish between regions of the system with different characteristics and clearly shows areas of strong attraction [47]. The interaction force for carotenoids with [P 4448 ]Cl can be seen in Figure S2 Table 2. Large interaction energies were obtained for the studied ILcarotenoid clusters, which indicates a high affinity of IL parts resulting from either the anion or cation with the carotenoid structures. For astaxanthin, β-carotene, and lutein, The total interaction energy (E int ) and energy gap (∆G) for the optimized [P 4448 ]Clcarotenoid structures were calculated with the strength of [P 4448 ]Cl-carotenoid interaction and are presented in Table 2. Large interaction energies were obtained for the studied IL-carotenoid clusters, which indicates a high affinity of IL parts resulting from either the anion or cation with the carotenoid structures. For astaxanthin, β-carotene, and lutein, [P 4448 ] + showed a larger E int than Cl −1 , suggesting that the interactions are mostly localized around the cation sites rather than the anion sites. In the case of [P 4448 ]Cl, the Eint value of IL-astaxanthin was the largest compared with others, whereas for astaxanthin, the solubility in [P 4448 ]Cl was the lowest. In a previous study, the solubilities of astaxanthin and lutein in deep eutectic solvent (DES)-based microemulsions showed a good linear relationship with the interaction energy of DES-carotenoid [45]. Therefore, the strong solubility of carotenoids in [P 4448 ]Cl were due to the van der Waals forces and hydrogen bonding that formed between them, and the IL cations play a major role in the interactions with the carotenoids.

Carotenoid Stability in [P 4448 ]Cl Aqueous Solution
Nowadays, natural pigments are becoming increasingly popular in the food and cosmetics industry. It was demonstrated that light, temperature, pH, and oxygen could affect the pigment stability in storage [48]. However, the effect of solvent nature on the pigment stability was always ignored in the previous literature. It was reported that 69% of astaxanthin was degraded after storage in hydroxypropyl-β-cyclodextrin at 4 • C for 120 h, and it was totally destroyed after storage at 50 • C for 32 h [49]. Storage of carotenoids at extreme pH values of <4 or >7 induces de-esterification and cis/trans isomerization of molecules [49]. In this study, the color stability and concentration change of carotenoids in [P 4448 ]Cl aqueous solution at different temperatures and water contents was explored. Each [P 4448 ]Cl aqueous solution containing astaxanthin, β-carotene, and lutein was stored in the dark for 12 days. Pictures of each sample stored from day 0 to day 12 are given in the Supplementary Materials (Figures S3-S7). Changes in ∆E, the concentration of carotenoids, and the relationship between ∆E and carotenoid concentration were measured to analyze the carotenoid stability in IL solutions.
An example of lutein stability in [P 4448 ]Cl aqueous solution (w water = 20%) at a temperature from 283.15 K to 338.15 K is shown in Figure 4.

Each [P4448]
Cl aqueous solution containing astaxanthin, β-carotene, and lutein was stored in the dark for 12 days. Pictures of each sample stored from day 0 to day 12 are given in the Supplementary Materials (Figures S3-S7). Changes in ΔE, the concentration of carotenoids, and the relationship between ΔE and carotenoid concentration were measured to analyze the carotenoid stability in IL solutions.
An example of lutein stability in [P4448]Cl aqueous solution (wwater = 20%) at a temperature from 283.15 K to 338.15 K is shown in Figure 4.  Figure S3 presents the appearance of a [P4448]Cl aqueous solutions containing astaxanthin, β-carotene, and lutein during storage. All the mixtures were clear and homogeneous when stored for 12 days. Most of the solutions (wwater > 30%) containing astaxanthin were red at 298.15 K to 328.15 K, then changed to orange at 338.15 K. For βcarotene and lutein, the solutions were light orange, and slightly visible changes were perceivable by the human eye.

Color Stability
The chromatic parameters (L*, a*, and b*) for all the solutions under different storage temperatures and water contents are shown in Figures S4 and S5, respectively. a* was the main parameter that reflects the color change of astaxanthin, and it decreased with increasing storage time. The value of b* is the main parameter that reflects the color change of β-carotene and lutein, and it also decreased with increasing storage time. ΔE was  Figure S3 presents the appearance of a [P 4448 ]Cl aqueous solutions containing astaxanthin, β-carotene, and lutein during storage. All the mixtures were clear and homogeneous when stored for 12 days. Most of the solutions (w water > 30%) containing astaxanthin were red at 298.15 K to 328.15 K, then changed to orange at 338.15 K. For β-carotene and lutein, the solutions were light orange, and slightly visible changes were perceivable by the human eye.

Color Stability
The chromatic parameters (L*, a*, and b*) for all the solutions under different storage temperatures and water contents are shown in Figures S4 and S5, respectively. a* was the main parameter that reflects the color change of astaxanthin, and it decreased with increasing storage time. The value of b* is the main parameter that reflects the color change of β-carotene and lutein, and it also decreased with increasing storage time. ∆E was calculated using Equation (3) and is given in Figure S6. The larger the value of ∆E, the less stable the color of the sample. The ∆E value of all samples increased significantly at the beginning of storage, while it increased sightly with the extension of storage time, indicating that the carotenoid degraded continuously during storage.
Moreover, the ∆E values of all [P 4448 ]Cl aqueous solutions containing astaxanthin, β-carotene, and lutein followed a temperature-dependent trend, whereby the ∆E value was obviously higher at a high temperature (338.15 K) compared to a low temperature (298.15 K). By contrast, the value of ∆E for the samples containing 10% water was slightly lower than that containing 50% water at 298.15 K. The result indicated that carotenoids in [P 4448 ]Cl aqueous solution have good stability at low temperature, and the effect of water content can be ignored. After 12 days of storage at 298.15 K, the ∆E value of [P 4448 ]Cl solution containing astaxanthin, β-carotene, and lutein was approximately 20, 45, and 30, respectively.

Carotenoid Degradation
The carotenoid concentration in all the solutions stored at different temperatures and water contents was also analyzed, and the data is shown in Figure S7. The degradation of astaxanthin, β-carotene, and lutein in all samples was related with the temperature and water content, whereby the degradation was more rapid at a high temperature (>318.15 K) or a high water content (>30%). After 12 days of storage at 298.15 K, the concentration of astaxanthin, β-carotene, and lutein in [P 4448 ]Cl solution (w water = 20%) decreased by approximately 13.4%, 42.3%, and 15.3%, respectively. It is worth noting that the carotenoid degradation in [P 4448 ]Cl solution was in agreement with the color change of the solution.
Moreover, the carotenoid degradation fitted a first-order kinetic reaction, expressed as follows [50]: ln (c/c 0 ) = −kt (1) where c and c 0 represent the carotenoids concentration at a specific storage time and at the initial time, respectively; t is the storage time (h); t 1/2 is the half-life (h); and k is the rate constant (h −1 ). High R 2 (>95%) values for all [P 4448 ]Cl solutions containing astaxanthin, β-carotene, and lutein were obtained, showing that the experimental data fit the first-order model. Similarly, the degradation and color change of astaxanthin in different atmosphere (air, vacuum) and storage temperatures (4, 15, 25 • C) and those of β-carotene in zein-carboxymethyl chitosan-tea polyphenol ternary composite nanoparticles stored in the dark at 5, 20, 37, and 60 • C for 7 days were found to follow a first-order kinetic reaction [51,52]. The kinetic parameters (k 1 and t 1/2(h) ) obtained from the first-order model are listed in Table 3. Generally, the samples stored at low temperatures and water contents showed a low degradation rate. The k 1 and t 1/2(h) values demonstrated that the stability of the carotenoids in the [P 4448 ]Cl solution followed the trend lutein > astaxanthin > β-carotene. Table 3. The rate constants (k 1 , h −1 ), t 1/2(h) and the relationship between the concentration of carotenoids and chromatic parameters.

Correlation between Concentration of Carotenoids and Color Parameters
For all [P 4448 ]Cl solutions containing carotenoids stored at different temperatures and water contents, varying degrees of color change and carotenoid degradation were observed. A previous study demonstrated a strong positive correlation between lutein color degradation and reduction in carotenoid content [53]. However, negative correlations were obtained for astaxanthin, astaxanthin ester, and lutein when stored in deep eutectic solvent-based microemulsions [45]. Hence, the relationship between the ∆E value and carotenoid content in the [P 4448 ]Cl solutions was determined, and the results are shown in Table 3. It can be seen that the chromatic parameters (L*, a*, and b*) and ∆E are significantly related to carotenoid concentration. The equations were able to correlate the carotenoid concentrations throughout the chromatic parameters, as R 2 values were around 0.87-0.98. The linear correlation demonstrate that the color parameters were an ideal index to conveniently monitor the carotenoid contents in IL solutions during storage.

IL Properties
The physicochemical properties, including density, pH, conductivity, and viscosity of the IL/water mixtures (wwater = 10% to 50%), were determined at atmospheric pressure and temperatures varying from T = (298.15 to 338.15 K) in steps of 10 K for the equal volume method. The samples were placed on a temperature-controlled chuck. The pH was determined using a pH meter (PHSJ-3F, Yidian Scientific Instrument Co., Ltd., Shanghai, China). The conductivity was determined using a conductivity meter (DDSJ-308A, Yidian Scientific Instrument Co., Ltd., Shanghai, China). The viscosity of the ILs was measured by a Malvern Kinexus Rheometer (Thermo, Waltham, MA, USA), and a parallel plate (diameter 20 mm) geometry was used with a fixed gap distance (1.0 mm) between the plates.

IL Properties
The physicochemical properties, including density, pH, conductivity, and viscosity of the IL/water mixtures (w water = 10% to 50%), were determined at atmospheric pressure and temperatures varying from T = (298.15 to 338.15 K) in steps of 10 K for the equal volume method. The samples were placed on a temperature-controlled chuck. The pH was determined using a pH meter (PHSJ-3F, Yidian Scientific Instrument Co., Ltd., Shanghai, China). The conductivity was determined using a conductivity meter (DDSJ-308A, Yidian Scientific Instrument Co., Ltd., Shanghai, China). The viscosity of the ILs was measured by a Malvern Kinexus Rheometer (Thermo, Waltham, MA, USA), and a parallel plate (diameter 20 mm) geometry was used with a fixed gap distance (1.0 mm) between the plates.

Carotenoid Solubility
The equilibrium solubility method was based on the saturation shake-flask solubility technique [42]. When the temperature reached the set value (298.15 K to 338.15 K), the carotenoid standard was added into the mixtures of IL and water (w water = 10% to 50%) until it was in excess. An SHA-CA Water bath thermostat shaker (Changzhou Aohua Biotechnology Co., Ltd., Changzhou, China) was used to stir the mixture for more than 24 h until it was dissolved and balanced. After reaching the equilibrium point, the saturated solution was centrifuged and subsequently filtered through a syringe filter (0.45 µm). The solution was diluted with ethanol and analyzed using a UV-Vis spectrophotometer. The concentration of the diluted solution was determined from the calibration curve.

Molecular Simulation
The PM7 semi-empirical method in the MOPAC program was used to optimize the initial structures of ILs, astaxanthin, β-carotene, and lutein. The clustering was performed using an energy of 0.5 kcal/mol and a conformational difference of 0.25 Å. The configuration optimization was carried out at the B3LYP-D3/6-31G* basis set level by using density functional theory (DFT). The first three conformations that were finally optimized were subjected to a single-point energy calculation at the B3LYP-D3/Def2-TZVP.

Color Changes
The color analysis samples were prepared by dissolving 1-2 mg of carotenoids into 20 mL of IL/water mixtures with ultrasound-assisted dissolution for 5 min. After filtering, the samples were incubated at different temperatures (298.15 K to 338.15 K) or different water contents (10% to 50%). To assessment of storage stability of different carotenoids in the IL/water mixtures, each sample was stored in the dark for 12 d. The L* (lightness), a*((+) red/(−) green), and b* ((+) yellow/(−) blue) color parameters were measured every 24 h using an automatism colorimeter (SC-80C, KangGuang Optical Instrument, CHN). The total color difference (∆E) was calculated with the following equation: where L * 0 , a * 0 , and b * 0 are the initial values of L*, a*, and b* color coordinates of the untreated samples, respectively. The color coordinates of samples that underwent storage or light treatment were L*, a*, and b*.

Concentration Changes
A 1-2 mg sample of carotenoids was dissolved into 20 mL of IL aqueous solution with ultrasound-assisted dissolution for 5 min. As storage time increased, the concentrations of astaxanthin, β-carotene, and lutein in the IL/water mixtures were determined by measuring the absorbance using a microplate reader (Synergy H1, USA). The carotenoid standards were dissolved in an anhydrous ethanol solution, and the standards were diluted with ethanol to different concentrations until the absorbance was between 0.2 and 1.0 absorbance units. After plotting the standard curve, the carotenoid concentrations could be derived from the absorbance.

Statistical Analysis
All experiments were performed in triplicate and the data were expressed as the mean ± standard deviation (SD). One-way analysis of variance (ANOVA) (Tukey's procedure at a confidence level of 95%) was applied, and significant differences were compared by Tukey's test at p < 0.05 using SPSS version 26.0.

Conclusions
Developing a new extraction solvent for carotenoids and studying their storage stability in solvents is beneficial for their application. In this study, ammonium-and phosphonium-based ILs were used as alternatives to organic solvents for astaxanthin, β-carotene, and lutein. The effects of the solvent nature, temperature, and water content on the physicochemical properties, carotenoid solubility, and storage stability were evaluated. The viscosity of all studied ILs was lower than 100 mPa·s −1 at 298.15-338.15 K at a water content of 20%. [P 4448 ]Cl presented the highest dissolving capacity at 338.15 K with a water content of 10%, which was higher than the organic solvent and imidazolium IL. The strong solubility of carotenoids in [P 4448 ]Cl was due to the interactions of IL cations with the carotenoids. Moreover, the solubility and stability of the carotenoids in [P 4448 ]Cl solution followed the trends lutein >> β-carotene > astaxanthin, and lutein > astaxanthin > β-carotene, respectively. The carotenoid degradation followed a first-order kinetic reaction, and the chromatic parameters (L*, a* and b*) and ∆E are significantly related to carotenoid concentration. Therefore, the color parameters were demonstrated as an ideal index to conveniently monitor the carotenoid contents in IL solutions during storage. This study provides a valuable reference for the extraction of carotenoids using ammoniumand phosphonium-based ILs, as well as the application of the extraction solution in the pharmaceutical, cosmeceutical, food, and feed industries.

Conflicts of Interest:
The authors declare no conflict of interest.